Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and...

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Chemistry 16.3

© Copyright Pearson Prentice Hall

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Limiting Reagent and Percent Yield

If a carpenter had two tabletops and seven table legs, he could only build one four-legged table. The number of table legs is the limiting factor in the construction of four-legged tables. Similarly, in chemistry, the amount of product made in a chemical reaction may be limited by the amount of one or more of the reactants.

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Limiting Reagent and Percent Yield >

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Limiting and Excess Reagents

Limiting and Excess Reagents

How is the amount of product in a reaction affected by an insufficient quantity of any of the reactants?

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Limiting Reagent and Percent Yield > Limiting and Excess Reagents

In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms.

The limiting reagent is the reagent that determines the amount of product that can be formed by a reaction.

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In the reaction of nitrogen and hydrogen, hydrogen is the limiting reagent. Nitrogen is the reagent that is not completely used up in the reaction. The reagent that is not used up is called the excess reagent.

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12.3

The Chemical Equation for the Preparation of Ammonia


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Animation 13

Apply the limiting reagent concept to the production of iron from iron ore.


SAMPLE PROBLEM

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Practice Problems for Sample Problem 12.7

Problem Solving 12.25 Solve Problem 25 with the help of an interactive guided tutorial.


SAMPLE PROBLEM

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Limiting Reagent and Percent Yield >

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Percent Yield

Percent Yield

What does the percent yield of a reaction measure?

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Limiting Reagent and Percent Yield > Percent Yield

The percent yield is a measure of the efficiency of a reaction carried out in the laboratory.

A batting average is actually a percent yield.

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• The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants.

• In contrast, the amount of product that actually forms when the reaction is carried out in the laboratory is called the actual yield.

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The percent yield is the ratio of the actual yield to the theoretical yield expressed as a percent.

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SAMPLE PROBLEM

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Section Quiz

-or-Continue to: Launch:

Assess students’ understanding of the concepts in Section

12.3 Section Quiz.

12.3.


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12.3 Section Quiz.

1. In the reaction 3NO2 + H2O 2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react?

a. 0.913 g

b. 0.667 g

c. 15.7 g

d. 1.37 g


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12.3 Section Quiz.

2. How many grams of H2O can be formed from 24.0 g O2 and 6.00 g H2?

a. 30.0 g

b. 27.0 g

c. 54.0 g

d. 13.5 g


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3. Octane burns according to the following equation.

2C8H18 + 25O2 16CO2 + 18H2O

What is the percent yield if 14.6 g of CO2 are produced when 5.00 g of

C8H18 are burned?

a. 106%

b. 94.8%

c. 34.2%

d. 62.5%

12.3 Section Quiz.


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Limiting Reagent and Percent Yield > Concept Map 12

Solve the Concept Map with the help of an interactive guided tutorial.

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Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and...

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